6th form transition pack
TRANSCRIPT
6th Form Transition Pack
QUALIFICATION A Level Chemistry
Teacher Name(s) Miss Jacks
Contact email(s) [email protected]
Exam board and link AQA https://www.aqa.org.uk/
Specification details specification code: 7405 QAN code: 601/5731/8
In addition, the transition pack may contain resources like PowerPoints, assessments and activities
for you to try at home over the summer.
We recommend you use Cornell Notes to prepare for your new course. Please see these videos to
help you develop the technique:
https://youtu.be/WtW9IyE04OQ
See the General Transition Pack where VESPA has been outlined for other ways of successfully taking
notes and organising the content of your studies effectively.
Please complete the activities in this booklet in readiness to begin your studies when we are told
Sixth Form may reopen. This will show us your commitment and may be used alongside your GCSE
grades and behaviour log as entry criteria – Sixth Form study is hard work and there are no short
cuts. Commitment to your studies is essential.
Good Luck and Stay Safe!
A-level Chemistry Do It Resources
Watch It.
The Magic of Chemistry - with Andrew Szydlo
Entropy (Order and Disorder) Energy BBC w/ Jim Al-Khalili HD
Chemical Curiosities: Surprising Science and Dramatic Demonstrations
Chemistry: A Volatile History with Jim Al-Khalili
Secrets of the Super Elements What is entropy? - Jeff Phillips
The genius of Mendeleev's periodic table - Lou Serico
Atom Jim Al-Khalili
Just How Small is an Atom?
Daniel Dulek: How big is a mole? (Not
the animal, the other one.) Jakob Magolan: A crash course in
organic chemistry
Royal Institution Christmas Lectures: The Modern Alchemist
Aaron Sams: How to speed up chemical reactions (and get a date)
Cathy Mulzer: The incredible chemistry powering your smartphone
Elizabeth Cox: Is fire a solid, a liquid, or a gas?
Royal Institution Chemistry Lectures
Read it
The Disappearing Spoon: And Other True Tales of Madness, Love, and the History of the World from the Periodic Table of the Elements (Hardcover) by Sam Kean
General Chemistry (Paperback) by Linus Pauling
Periodic Tales: The Curious Lives of the Elements (Hardcover) by Hugh Aldersey-Williams
Elements: A Visual Exploration of Every Known Atom in the Universe (Hardcover) by Theodore Gray
Uncle Tungsten (Paperback) by Oliver Sacks
A Chemical History of a Candle (Paperback) by Michael Faraday
Napoleon's Buttons: How 17 Molecules Changed History (Hardcover) by Penny Le Couteur
Stuff Matters: Exploring the Marvelous Materials That Shape Our Man-Made World (Hardcover) by Mark Miodownik
A Short History of Chemistry (Science Study) by Isaac Asimov
The Sweetness at the Bottom of the Pie (Flavia de Luce, #1) by Alan Bradley
The Poisoner's Handbook: Murder and the Birth of Forensic Medicine in Jazz Age New York (Hardcover) by Deborah Blum
Bad Science: Quacks, Hacks, and Big Pharma Flacks by Ben Goldacre
Google it
https://www.youtube.com/user/MaChemGuy
https://www.chemguide.co.uk
http://www.knockhardy.org.uk/sci.htm
http://www.periodicvideos.com
https://edu.rsc.org
http://www.a-levelchemistry.co.uk
https://www.senecalearning.com/blog/a-level-
chemistry-revision/ https://studywise.co.uk/a-level-revision/chemistry/
https://chemrevise.org
https://www.rsc.org/periodic-table/
https://www.innovativeeducation.org
https://snaprevise.co.uk
Study It (for Free)
A Huge Library of Free Chemistry Textbooks AQA Chemistry Year 1 (AS) Chemistry Head Start to A-level Chemistry (Kindle)
Chemistry 2e Textbook Cambridge International AS and A-level Chemistry
AQA Chemistry A-level 2nd Edition
Listen to it
The Infinite Monkey Cage https://www.bbc.co.uk/programmes/b00snr0w/
episodes/downloads
Chemistry World Podcast https://www.chemistryworld.c
om/podcasts
The Guardian - Science weekly https://www.theguardian.com/science/
series/science
BBC Science and Nature https://www.bbc.co.uk/podcasts/category/scien
ceandnature
Chemistry for Life https://player.fm/series/chemi
stry-for-your-life
The Naked Scientist https://audioboom.com/channel/naked
scientistspodcast
GCSE to A-Level Chemistry
Transition Work
Instructions
You MUST complete all GCSE questions. This is to help you recap and retrieve vital knowledge you have learned during your GCSE course that provides the foundation for A-Level Chemistry to build upon.
Use your normal GCSE revision resources to help you complete them, but here are some suggestions:
www.tassomai.com
www.senecalearning.com
www.bitesize.com
Youtube - Free Science Lessons
Youtube - Primrose Kitten
You MUST attempt the A-Level Questions. They are accessible to you with the GCSE content you have – you might just need to think outside the box a bit and stretch yourself! This gives insight into the style of questions at A-Level and shows the jump is not that large if you are fully prepped with all of your GCSE knowledge
CGP – ‘Head start to Chemistry’ and ‘Essential Maths Skills’ books
MaChemGuy – Prepare for A-Level Chemistry
ASFC Chemistry – Starting A-Level Chemistry
You MUST bring this to your first Chemistry Lesson in Year 12 and give it to your teacher
GCSE to A-Level Chemistry – Transition Work
Atomic Structure
GCSE questions
Q1. This question is about the structure of the atom.
(a) Complete the sentences. Choose answers from the box. Each word may be used once, more than once, or not at all.
electron ion neutron
nucleus proton
The centre of the atom is the _______________________ .
The two types of particle in the centre of the atom are the proton and the _______________________ .
James Chadwick proved the existence of the _______________________ .
Niels Bohr suggested particles orbit the centre of the atom. This type of particle is the ________________ .
The two types of particle with the same mass are the neutron and the _______________________ . (5)
The table below shows information about two isotopes of element X.
Mass number Percentage (%) abundance
Isotope 1 63 70
Isotope 2 65 30
(b) Calculate the relative atomic mass (Ar) of element X using the equation:
Use the table above. Give your answer to 1 decimal place.
________________________________________________________________________________________
__________________________________________________________Ar = _________________ (2)
(c) Suggest the identity of element X. Use the periodic table.
Element X is _________________________________________________________________________(1)
(d) The radius of an atom of element X is 1.2 × 10−10 m
The radius of the centre of the atom is the radius of the atom.
Calculate the radius of the centre of an atom of element X. Give your answer in standard form.
________________________________________________________________________________________
________________________________________________________________________________________
_______________________________________________Radius = ___________________ m (2)
Q2. The diagram below represents different models of the atom.
(a) Which diagram shows the plum pudding model of the atom? Tick one box.
(1)
(b) Which diagram shows the model of the atom developed from the alpha particle scattering experiment? Tick one box.
(1)
(c) Which diagram shows the model of the atom resulting from Bohr’s work? Tick one box.
(1)
(d) Define the mass number of an atom.
_______________________________________________________________________________________
_________________________________________________________________________________(1)
(e) Element X has two isotopes. Their mass numbers are 69 and 71
The percentage abundance of each isotope is:
• 60% of 69X • 40% of 71X
Estimate the relative atomic mass of element X. Tick one box.
< 69.5
Between 69.5 and 70.0
Between 69.5 and 70.0
Between 70.0 and 70.5
> 70.5
(1) A-Level question to give a go!
Q1. Which of these correctly shows the numbers of sub-atomic particles in a 41K+ ion?
Number of electrons
Number of protons
Number of neutrons
A 19 19 20
B 18 20 21
C 18 19 22
D 19 18 23
(Total 1 mark)
Q2. Magnesium exists as three isotopes: 24Mg, 25Mg and 26Mg
(a) In terms of sub-atomic particles, state the difference between the three isotopes of magnesium.
_______________________________________________________________________________________
_____________________________________________________________________________________(1)
(b) State how, if at all, the chemical properties of these isotopes differ.
Give a reason for your answer.
Chemical properties ______________________________________________________________________
Reason
_______________________________________________________________________________________
_____________________________________________________________________________________(2)
Amount of Substance
GCSE questions
Q3. A student investigated the reactions of copper carbonate and copper oxide with dilute hydrochloric acid. In both reactions one of the products is copper chloride.
(a) A student wanted to make 11.0 g of copper chloride.
The equation for the reaction is:
CuCO3 + 2HCl → CuCl2 + H2O + CO2
Relative atomic masses, Ar: H = 1; C = 12; O = 16; Cl = 35.5; Cu = 63.5
Calculate the mass of copper carbonate the student should react with dilute hydrochloric acid to make 11.0 g of copper chloride.
________________________________________________________________________________________
________________________________________________________________________________________
___________________________Mass of copper carbonate = _________________________ g (4)
(b) The percentage yield of copper chloride was 79.1 %. Calculate the mass of copper chloride the student actually produced.
________________________________________________________________________________________
______________________________Actual mass of copper chloride produced = ____________ g (2)
(c) Look at the equations for the two reactions:
Reaction 1 CuCO3(s) + 2HCl(aq) → CuCl2(aq) + H2O(l) + CO2(g)
Reaction 2 CuO(s) + 2HCl(aq) → CuCl2(aq) + H2O(l)
Reactive formula masses: CuO = 79.5; HCl = 36.5; CuCl2 = 134.5; H2O = 18
The percentage atom economy for a reaction is calculated using:
Calculate the percentage atom economy for Reaction 2.
_________________________________________________________________________________________
_________________________________________________________________________________________
____________________________Percentage atom economy = ________________________ % (3)
(d) The atom economy for Reaction 1 is 68.45 %. Compare the atom economies of the two reactions for making copper chloride. Give a reason for the difference.
__________________________________________________________________________________(1)
A-Level question to give a go!
Q3. Ethanol can be made from glucose by fermentation.
C6H12O6 → 2C2H5OH + 2CO2
In an experiment, 268 g of ethanol (Mr = 46.0) were made from 1.44 kg of glucose (Mr = 180.0). What is the percentage yield?
A 18.6%
B 36.4%
C 51.1%
D 72.8%
(Total 1 mark)
Q4. A gas cylinder contains 5.0 kg of propane. How many propane molecules are in the cylinder? The Avogadro constant, L = 6.022 × 1023 mol–1
A 6.8 × 1022
B 7.2 × 1022
C 6.8 × 1025
D 7.2 × 1025
(Total 1 mark)
Bonding
GCSE questions
Q4. Figure 1 shows the structure of five substances.
(a) Which diagram shows a gas? Tick (✔) one box.
A
B
C D E
(1)
(b) Which diagram shows the structure of diamond? Tick (✔) one box.
A
B
C D E
(1)
(c) Which diagram shows a metallic structure? Tick (✔) one box.
A
B
C D E
(1)
(d) Which diagram shows a polymer? Tick (✔) one box.
A
B
C D E
(1)
(e) A chlorine atom has 7 electrons in the outer shell.
Two chlorine atoms covalently bond to form a chlorine molecule, Cl2
Figure 2 is a dot and cross diagram showing the outer shells and some electrons in a chlorine molecule.
Complete the dot and cross diagram. Show only the electrons in the outer shell.
(1)
(f) What is the reason for chlorine’s low boiling point? Tick (✔) one box.
Strong covalent bonds
Strong forces between molecules
Weak covalent bonds
Weak forces between molecules
(1)
Figure 3 represents the structure of manganese oxide. Manganese oxide is an ionic compound.
(g) Determine the empirical formula of manganese oxide. Use Figure 3.
_______________________________________________________________________________________
__________________________________________Empirical formula = ______________________ (1)
(h) Why does manganese oxide conduct electricity as a liquid? Tick (✔) one box.
Atoms move around in the liquid
Electrons move around in the liquid
Ions move around in the liquid
Molecules move around in the liquid
(1)
Q5. This question is about structure and bonding.
(a) Complete the dot and cross diagram to show the covalent bonding in a nitrogen molecule, N2
Show only the electrons in the outer shell.
(2)
(b) Explain why nitrogen is a gas at room temperature. Answer in terms of nitrogen’s structure.
_______________________________________________________________________________________
_______________________________________________________________________________________
_______________________________________________________________________________________
____________________________________________________________________________(3)
(c) Graphite and fullerenes are forms of carbon. Graphite is soft and is a good conductor of electricity.
Explain why graphite has these properties. Answer in terms of structure and bonding.
_______________________________________________________________________________________
_______________________________________________________________________________________
_______________________________________________________________________________________
_______________________________________________________________________________________
____________________________________________________________________________________(4)
A-Level question to give a go!
Q5. Which is the correct crystal structure for the substance named?
Substance Structure
A Iodine Simple molecular
B Diamond Ionic
C Sodium chloride Giant covalent
D Graphite Metallic
(Total 1 mark)
Q6. What is the formula of calcium nitrate(V)?
A CaNO3
B Ca(NO3)2
C Ca2NO2
D Ca(NO2)2
(Total 1 mark)
Q7. The table shows some data about the elements bromine and magnesium.
Element Melting point / K Boiling point / K
Bromine 266 332
Magnesium 923 1383
In terms of structure and bonding explain why the boiling point of bromine is different from that of magnesium. Suggest why magnesium is a liquid over a much greater temperature range compared to bromine.
________________________________________________________________________________________
________________________________________________________________________________________
________________________________________________________________________________________
________________________________________________________________________________________
________________________________________________________________________________________
________________________________________________________________________________________
________________________________________________________________________________________
________________________________________________________________________________________
________________________________________________________________________________________
________________________________________________________________________________________
____________________________________________________________________________(Total 5 marks)
Energetics GCSE questions
Q6. Methane (CH4) is used as a fuel.
(a) Methane burns in oxygen.
(i) The diagram below shows the energy level diagram for the complete combustion of methane.
Draw and label arrows on the diagram to show:
• the activation energy • the enthalpy change, ∆H.
(2)
(ii) Complete and balance the symbol equation for the complete combustion of methane.
CH4 + _____ CO2 + _____ (2)
(ii) Explain why, in terms of the energy involved in bond breaking and bond making, the combustion of methane is exothermic.
________________________________________________________________________________________
________________________________________________________________________________________
________________________________________________________________________________________
_________________________________________________________________________(3)
(b) Methane reacts with chlorine in the presence of sunlight. The equation for this reaction is:
Some bond dissociation energies are given in the table.
Bond Bond dissociation energy
in kJ per mole
C−H 413
C−Cl 327
Cl−Cl 243
H−Cl 432
(i) Show that the enthalpy change, ∆H, for this reaction is −103 kJ per mole.
________________________________________________________________________________________
________________________________________________________________________________________
________________________________________________________________________________________
_________________________________________________________________________(3)
(ii) Methane also reacts with bromine in the presence of sunlight.
This reaction is less exothermic than the reaction between methane and chlorine.
The enthalpy change, ∆H, is −45 kJ per mole.
What is a possible reason for this? Tick ( ) one box.
CH3Br has a lower boiling point than CH3Cl
The C−Br bond is weaker than the C−Cl bond.
The H−Cl bond is weaker than the H−Br bond.
Chlorine is more reactive than bromine.
(1) A-Level question to give a go!
Q8. Calculate the enthalpy change, in kJ, for this dissociation of mole of propan-1-ol.
C3H7OH(g) ⟶ 3C(g) + 8H(g) + O(g)
Mean bond dissociation enthalpy / kJ mol−1 412 348 360 463
A −4751
B −4403
C +4403
D +4751
(Total 1 mark)
Q9. Hydrogen is produced by the reaction of methane with steam. The reaction mixture reaches a state of dynamic equilibrium.
CH4(g) + H2O(g) ⇌ CO(g) + 3H2(g) ∆H = +206 kJ mol−1
Some enthalpy data is given in the table.
Bond C–H O–H H–H C≡H Bond enthalpy /
kJ mol−1 413 463 436 To be calculated
Use the information in the table and the stated enthalpy change to calculate the missing bond enthalpy.
A
234
B 1064
C 1476
D 1936
(Total 1 mark)
Kinetics
GCSE questions
Q7. When sodium thiosulfate solution reacts with dilute hydrochloric acid, the solution becomes cloudy.
The equation for the reaction is:
Na2S2O3(aq) + 2 HCl(aq) ⟶ 2 NaCl(aq) + SO2(g) + H2O(l) + S(s)
Some students used this reaction to investigate the effect of concentration on rate of reaction. The table shows the students’ results.
Concentration of sodium thiosulfate solution in mol / dm3
Time for cross to become no longer visible in s
0.020 170
0.040 90
0.060 82
0.080 42
0.100 34
0.120 30
0.140 28
(a) Plot the data from the table above on the graph below. Draw a line of best fit.
(3)
The students repeated the investigation two more times. They obtained similar results each time.
(b) The students analysed their results to give a conclusion and an explanation for their investigation.
Conclusion: ‘The higher the concentration, the lower the rate of reaction.’
Explanation: ‘At higher concentrations, the particles have more energy, so they are moving faster. Therefore the collisions are more energetic.’
The students are not correct.
Give a correct conclusion and explanation for the results of the investigation.
Conclusion __________________________________________________________________________
____________________________________________________________________________________
Explanation ___________________________________________________________________________
_______________________________________________________________________________________
_______________________________________________________________________________________
_____________________________________________________________________________________(3)
(c) A solution containing 0.18 g of sodium thiosulfate reacts with dilute hydrochloric acid in 2 minutes.
Calculate the mean rate of reaction in g / s. Give your answer in standard form.
_______________________________________________________________________________________
_______________________________________________________________________________________
_________________________________________Mean rate of reaction = ____________________ g / s (3)
A-Level question to give a go!
Q10. Line X in the diagram represents the volume (V) of gas formed with time (t) in a reaction between an excess of magnesium and aqueous sulfuric acid.
Which line represents the volume of hydrogen formed, at the same temperature and pressure, when the concentration of sulfuric acid has been halved?
A
B
C
D
(Total 1 mark)
Q11. The gas-phase reaction between hydrogen and chlorine is very slow at room temperature.
H2(g) + Cl2(g) → 2HCl(g)
(a) Define the term activation energy.
________________________________________________________________________________________
______________________________________________________________________________________(2)
(b) Give one reason why the reaction between hydrogen and chlorine is very slow at room temperature.
________________________________________________________________________________________
______________________________________________________________________________________(1)
(c) Explain why an increase in pressure, at constant temperature, increases the rate of reaction between hydrogen and chlorine.
________________________________________________________________________________________
______________________________________________________________________________________(2)
(d) Explain why a small increase in temperature can lead to a large increase in the rate of reaction between hydrogen and chlorine.
________________________________________________________________________________________
______________________________________________________________________________________(2)
(e) Give the meaning of the term catalyst.
________________________________________________________________________________________
______________________________________________________________________________________(1)
(f) Suggest one reason why a solid catalyst for a gas-phase reaction is often in the form of a powder.
______________________________________________________________________________________(1)
Chemical Equilibria, Le Chatelier’s Principle and Kc
GCSE questions
Q8. In industry ethanol is produced by the reaction of ethene and steam at 300°C and 60 atmospheres pressure using a catalyst.
The equation for the reaction is: C2H4 (g) + H2O (g) C2H5OH (g)
(a) The forward reaction is exothermic.
Use Le Chatelier’s Principle to predict the effect of increasing temperature on the amount of ethanol produced at equilibrium. Give a reason for your prediction.
________________________________________________________________________________________
______________________________________________________________________________________(2)
(b) Explain how increasing the pressure of the reactants will affect the amount of ethanol produced at equilibrium.
________________________________________________________________________________________
______________________________________________________________________________________(2)
A-Level question to give a go!
Q12. Which statement is not correct about the industrial preparation of ethanol by the hydration of ethene at 300 °C?
C2H4(g) + H2O(g) ⇌ C2H5OH(g) ∆H = –46 kJ mol–1
A The reaction is catalysed by an acid.
B The higher the pressure, the higher the equilibrium yield of ethanol.
C The higher the temperature, the higher the equilibrium yield of ethanol.
D A low equilibrium yield of ethanol is acceptable because unreacted ethene is recycled.
(Total 1 mark)
Q13. The forward reaction in this equilibrium is endothermic
COCl2 (g) ⇌ CO(g) + Cl2 (g)
Which statement is correct?
A If the total pressure is increased at constant temperature, the proportion of COCl2 in the equilibrium mixture will decrease
B Use of a catalyst will increase the proportion of COCl2 in the equilibrium mixture at constant temperature and pressure
C Reducing the equilibrium concentration of CO will increase the value of the equilibrium constant
D Raising the temperature from 373 K to 473 K will increase the value of the equilibrium constant
(Total 1 mark)
Oxidation, Reduction and Redox equations
GCSE questions
Q9. This question is about halogens and their compounds. (a) What is the ionic equation for the reaction of chlorine with potassium iodide? Tick one box.
Cl2 + 2K → 2KCl
2I⁻ + Cl2 → I2 + 2Cl⁻
I⁻ + Cl → I + Cl⁻
I⁻ + K+ → KI (1)
Q10. Titanium is a transition metal.
Titanium is extracted from titanium dioxide in a two-stage industrial process.
Stage 1 TiO2 + 2 C + 2 Cl2 ⟶ TiCl4 + 2 CO
Stage 2 TiCl4 + 4 Na ⟶ Ti + 4 NaCl
In Stage 2, sodium displaces titanium from titanium chloride.
(a) Sodium atoms are oxidised to sodium ions in this reaction. Why is this an oxidation reaction?
___________________________________________________________________________________(1)
(b) Complete the half equation for the oxidation reaction.
Na ⟶ ____________ + ____________ (1)
A-Level question to give a go!
Q14. In which reaction is the metal oxidised?
A
2Cu2+ + 4I– 2CuI + I2
B [Fe(H2O)6]3+ + Cl– [Fe(H2O)5(Cl)]2+ + H2O
C [CoCl4]2– + 6H2O [Co(H2O)6]2+ + 4Cl–
D Mg + S MgS
(Total 1 mark)
Periodicity
GCSE questions
Q11. This question is about metals.
(a) Which unreactive metal is found in the Earth as the metal itself? Tick ( ) one box
aluminium
gold
magnesium
(1)
(b) Complete the sentence.
Aluminium is an element because aluminium is made of only one type of _________________________ . (1)
(c) Figure 1 shows the electronic structure of an aluminium atom.
(i) Use the correct words from the box to complete the sentence.
electrons ions protons neutrons shells
The nucleus of an aluminium atom contains _______________ and _______________ . (2)
(ii) Complete the sentence.
In the periodic table, aluminium is in Group ___________________ (1)
(d) Aluminium is used for kitchen foil. Figure 2 shows a symbol on a box of kitchen foil.
The symbol means that aluminium can be recycled. It does not show the correct chemical symbol for aluminium.
(i) What is the correct chemical symbol for aluminium? ___________________________ . (1)
(ii) Give two reasons why aluminium should be recycled.
________________________________________________________________________________________
______________________________________________________________________________________(2)
(e) Aluminium has a low density, conducts electricity and is resistant to corrosion.
Which one of these properties makes aluminium suitable to use as kitchen foil? Give a reason for your answer.
______________________________________________________________________________________
______________________________________________________________________________________
____________________________________________________________________________________(2)
A-Level question to give a go!
Q15. Which of the following is a correct statement about the trend in atomic radius across Period 3 of the Periodic Table?
A radius increases because the atoms have more electrons
B radius decreases because nuclear charge increases
C radius increases because shielding (screening) increases
D radius decreases because shielding (screening) decreases
(Total 1 mark)
Group 2 – The Alkaline Earth Metals
GCSE questions
Q12. This question is about compounds.
(a) The table gives information about the solubility of some compounds.
Soluble compounds
All potassium and sodium salts
All nitrates
Chlorides, bromides and iodides, except those of silver and lead
Use information from the table to answer these questions.
(i) Name a soluble compound that contains silver ions.
______________________________________________________________________________________(1)
(ii) Name a soluble compound that contains carbonate ions.
______________________________________________________________________________________(1)
(b) Metal oxides react with acids to make salts. What type of compound is a metal oxide?
______________________________________________________________________________________(1)
(c) Lead nitrate solution is produced by reacting lead oxide with nitric acid.
(i) State how solid lead nitrate can be obtained from lead nitrate solution.
_________________________________________________________________________________________
_______________________________________________________________________________________(1)
(ii) Balance the equation for the reaction.
PbO + HNO3 Pb(NO3)2 + H2O (1)
(iii) Give the total number of atoms in the formula Pb(NO3)2
_____________________________________________________________________________________(1)
A-Level question to give a go!
Q16. (a) Nickel is a metal with a high melting point.
(i) Explain, in terms of its structure and bonding, why nickel has a high melting point.
_______________________________________________________________________________________
_______________________________________________________________________________________
_______________________________________________________________________________________
_____________________________________________________________________________________(2)
(ii) Draw a labelled diagram to show the arrangement of particles in a crystal of nickel. In your answer, include at least six particles of each type.
(2)
(iii) Explain why nickel is ductile (can be stretched into wires).
_______________________________________________________________________________________
_____________________________________________________________________________________(1)
Group 7 – The Halogens
GCSE questions
Q13. The halogens are elements in Group 7.
(a) Bromine is in Group 7.
Give the number of electrons in the outer shell of a bromine atom. _______________________________(1)
(b) Bromine reacts with hydrogen. The gas hydrogen bromide is produced.
What is the structure of hydrogen bromide? Tick one box.
Giant covalent
Ionic lattice
Metallic structure
Small molecule
(1)
(c) What is the formula for fluorine gas? Tick one box.
F
F2
F2
2F
(1)
A student mixes solutions of halogens with solutions of their salts.
The table below shows the student’s observations.
Potassium chloride
(colourless) Potassium bromide
(colourless) Potassium iodide
(colourless)
Chlorine (colourless)
Solution turns orange Solution turns brown
Bromine (orange) No change Solution turns brown
Iodine (brown) No change No change
(d) Explain how the reactivity of the halogens changes going down Group 7. Use the results in the table above.
______________________________________________________________________________________
______________________________________________________________________________________
______________________________________________________________________________________
____________________________________________________________________________________(3)
A-Level question to give a go!
Q17. An aqueous solution of a white solid gives a yellow precipitate with aqueous silver nitrate. The formula of the white solid could be
A AgBr
B AgI
C NaBr
D NaI (Total 1 mark)
Q18. What will you see when a solution of silver nitrate is added to a solution containing bromide ions, and concentrated aqueous ammonia is added to the resulting mixture?
A a white precipitate soluble in concentrated aqueous ammonia
B a white precipitate insoluble in concentrated aqueous ammonia
C a cream precipitate soluble in concentrated aqueous ammonia
D a yellow precipitate insoluble in concentrated aqueous ammonia (Total 1 mark)
Introduction to Organic Chemistry
GCSE questions
Q14. Scientists found that a compound contained:
22.8% sodium; 21.8% boron; and 55.4% oxygen.
Use the percentages to calculate the empirical formula of the compound.
Relative atomic masses (A r): B = 11; O = 16; Na = 23
To gain full marks you must show all your working.
______________________________________________________________________________________
______________________________________________________________________________________
______________________________________________________________________________________
______________________________________________________________________________________
______________________________________________________________________________________
______________________________________________________________________________________
______________________________________________________________________________________
______________________________________________________________________________________
______________________________________________________________________________________
__________________________Empirical formula = ________________________________(Total 5 marks)
A-Level question to give a go!
Q19. An organic compound is found to contain 40.0% carbon, 6.7% hydrogen and 53.3% oxygen.
Which of the following compounds could this be?
A
Ethanol
B Ethanoic acid
C Methanol
D Methanoic acid
(Total 1 mark)
Alkanes
GCSE questions
Q15. This question is about hydrocarbons.
The table gives information about four hydrocarbons. The hydrocarbons are four successive members of a homologous series.
Hydrocarbon Formula Boiling point in °C
A C4H10 0
B 36
C C6H14 69
D C7H16 98
(a) What is the formula of hydrocarbon B? Tick (✔) one box.
C4H12
C5H12
C5H12
C6H12
(1)
(b) What is the simplest ratio of carbon : hydrogen atoms in a molecule of hydrocarbon A?
Ratio = 2 : _______ (1)
(c) Which hydrocarbon is a gas at room temperature (25 °C)? Tick (✔) one box.
A
B
C D
(1)
(d) Which hydrocarbon is most flammable? Tick (✔) one box.
A
B
C D
(1)
(e) Which two substances are produced when a hydrocarbon completely combusts in air? Tick (✔) two boxes.
Carbon
Carbon dioxide
Hydrogen
Sulfur dioxide
Water
(2)
The diagram shows the displayed structure of a hydrocarbon molecule.
(f) What is the name of the hydrocarbon in the diagram above? Tick (✔) one box.
Butane
Ethane
Methane
Propane
(1)
Q16. This question is about hydrocarbons.
(a) The names and formulae of three hydrocarbons in the same homologous series are:
Ethane C2H6
Propane C3H8
Butane C4H10
The next member in the series is pentane. What is the formula of pentane?
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(b) Which homologous series contains ethane, propane and butane? Tick one box.
Alcohols
Alkanes
Alkenes
Carboxylic acids
(1)
(c) Propane (C3H8) is used as a fuel. Complete the equation for the complete combustion of propane.
C3H8 + 5O2 → 3 _______________ + 4 _________________ (2)
(d) Octane (C8H18) is a hydrocarbon found in petrol. Explain why octane is a hydrocarbon.
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(e) The table below gives information about the pollutants produced by cars using diesel or petrol as a fuel.
Fuel Relative amounts of pollutants
Oxides of Nitrogen Particulate matter Carbon dioxide
Diesel 31 100 85
Petrol 23 0 100
Compare the pollutants from cars using diesel with those from cars using petrol.
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(f) Pollutants cause environmental impacts. Draw one line from each pollutant to the environmental impact caused by the pollutant.
Pollutant Environmental impact
caused by the pollutant
Acid rain
Oxides of nitrogen Flooding
Global dimming
Particulate matter Global warming
Photosynthesis
(2) A-Level question to give a go!
Q20. Which correctly represents an incomplete combustion of pentane?
A C5H12 + 8O2 ⟶ 5CO2 + 6H2O
B C5H12 + 8O2 ⟶ 4CO + CO2 + 6H2O
C C5H12 + 6O2 ⟶ 4CO + CO2 + 6H2O
D C5H12 + 5O2 ⟶ 4CO + CO2 + 4H2O + 2H2
(Total 1 mark)
Q21. Tetradecane (C14H30) is an alkane found in crude oil. When tetradecane is heated to a high temperature, one molecule of tetradecane decomposes to form one molecule of hexane and three more molecules.
Which of the following could represent this reaction?
A C14H30 → C6H14 + C4H8 + 2C2H4
B C14H30 → C6H14 + C6H12 + C2H4
C C14H30 → C5H12 + 3C3H6
D C14H30 → C6H14 + C2H6 + 2C3H6
(Total 1 mark)
Q22. Petrol contains saturated hydrocarbons. Some of the molecules in petrol have the molecular formula C8H18 and are referred to as octanes. These octanes can be obtained from crude oil by fractional distillation and by cracking suitable heavier fractions.
Petrol burns completely in a plentiful supply of air but can undergo incomplete combustion in a car engine.
(a) State the meaning of both the words saturated and hydrocarbon as applied to the term saturated hydrocarbon. Name the homologous series to which C8H18 belongs.
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(b) Outline the essential features of the fractional distillation of crude oil that enable the crude oil to be separated into fractions.
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Halogenalkanes
GCSE questions
Q17. During the test for unsaturation – a haloalkane is made. Describe the test for unsaturation
Test ________________________________________________________________________________
Result _____________________________________________________________________________(2)
Alkenes
GCSE questions
Q18. This question is about organic compounds. Hydrocarbons can be cracked to produce smaller molecules.
The equation shows the reaction for a hydrocarbon, C18H38
C18H38 → C6H14 + C4H8 + 2 C3H6 + C2H4
(a) Which product of the reaction shown is an alkane? Tick one box.
C2H4
C3H6
C4H8
C6H14 (1)
(b) The table below shows the boiling point, flammability and viscosity of C18H38 compared with the other hydrocarbons shown in the equation.
Boiling point Flammability Viscosity
A highest lowest highest
B highest lowest lowest
C lowest highest highest
D lowest highest lowest
Which letter, A, B, C or D, shows how the properties of C18H38 compare with the properties of C2H4, C3H6, C4H8 and C6H14? Tick one box.
A
B
C
D (1)
(c) The hydrocarbon C4H8 was burnt in air. Incomplete combustion occurred.
Which equation, A, B, C or D, correctly represents the incomplete combustion reaction?
A C4H8 + 4O → 4CO + 4H2
B C4H8 + 4O2 → 4CO + 4H2O
C C4H8 + 6O2 → 4CO2 + 4H2O
D C4H8 + 8O → 4CO2 + 4H2
Tick one box.
A
B
C
D
(1)
(d) Propanoic acid is a carboxylic acid. Which structure, A, B, C or D, shows propanoic acid?
Tick one box.
A
B
C
D
(1)
(e) Propanoic acid is formed by the oxidation of which organic compound? Tick one box.
Propane
Propene
Propanol
Polyester
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Q19. A molecule of ethene (C2H4) is represented as:
(a) A sample of ethene is shaken with bromine water. Complete the sentence.
The bromine water turns from orange to _____________________________________________________(1)
(b) Most ethene is produced by the process of cracking.
(i) Decane (C10H22) can be cracked to produce ethene (C2H4) and one other product.
Complete the equation to show the formula of the other product.
C10H22 C2H4 + _____________ (1)
(c) Many molecules of ethene join together to produce poly(ethene).
(i) Complete the structure of the polymer in the equation.
(2)
(ii) Some carrier bags are made from poly(ethene). Some carrier bags are made from cornstarch.
Suggest two benefits of using cornstarch instead of poly(ethene) to make carrier bags.
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A-Level question to give a go!
Q23. Consider the following reactions.
(a) State the type of reaction in Reaction 3. Give the name of substance X.
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Alcohols
GCSE questions
Q20. The diagrams represent two compounds, A and B.
Compound A Compound B
(a) (i) Compound B is an alcohol. Name compound B.
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(ii) Use the correct answer from the box to complete the sentence.
burned decomposed oxidised
To form compound A, compound B is ____________________________________________________(1)
(iii) Compounds A and B are both colourless liquids.
A test tube contains a colourless liquid, which could be either compound A or compound B. Describe a simple chemical test to show which compound, A or B, is in the test tube.
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A-Level question to give a go!
Q24. A group of students wanted to produce a biofuel to power the central heating system in their school. They collected scraps of fruits and vegetables from the kitchens and fermented them with yeast, in the absence of air, in order to produce ethanol.
The aqueous mixture was filtered to remove the remaining solids.
The students then set up the apparatus shown in the diagram below and placed the aqueous mixture in the round bottomed flask.
(a) Describe how the students would use this apparatus to collect a sample of ethanol. Include in your answer the functions of the parts of the apparatus labelled A, B and C.
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Organic Analysis
GCSE questions Q21. Four bottles of chemicals made in the 1880s were found recently in a cupboard during a Health and Safety inspection at Lovell Laboratories.
Sodium carbonate sodium chloride sodium nitrate sodium sulfate
The chemical names are shown below each bottle. (a) You are provided with the following reagents:
• aluminium powder • barium chloride solution acidified with dilute hydrochloric acid • dilute hydrochloric acid • silver nitrate solution acidified with dilute nitric acid • sodium hydroxide solution. • limewater • red litmus paper
(i) Describe tests that you could use to show that these chemicals are correctly named.
In each case give the reagent(s) you would use and state the result.
Test and result for carbonate ions:
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Test and result for chloride ions:
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Test and result for nitrate ions:
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Test and result for sulfate ions:
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(ii) Suggest why a flame test would not distinguish between these four chemicals.
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(b) Instrumental methods of analysis linked to computers can be used to identify chemicals. Give two advantages of using instrumental methods of analysis.
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A-Level question to give a go!
Q25. Consider the following scheme of reactions.
(a) High resolution mass spectrometry of a sample of propane indicated that it was contaminated with traces of carbon dioxide.
Use the data in the table to show how precise Mr values can be used to prove that the sample contains both of these gases.
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GCSE to A-Level Chemistry – Skills Transition
Balancing Equations
Use this method to help you https://www.youtube.com/watch?v=ab0gYBdHU-k
GCSE questions
Q1. (a) Balance these chemical equations.
(i) H2 + O2 → H2O (1)
(ii) Al + O2 → Al2O3 (1)
(b) Briefly explain why an unbalanced chemical equation cannot fully describe a reaction.
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Q2. The following passage was taken from a chemistry textbook.
Germanium is a white, shiny, brittle element. It is used in the electronics industry because it is able to conduct a small amount of electricity. It is made from germanium oxide obtained from flue dusts of zinc and lead smelters. The impure germanium oxide from the flue dusts is changed into germanium by the process outlined below.
STEP 1 The germanium oxide is reacted with hydrochloric acid to make germanium tetrachloride. This is a volatile liquid in which the germanium and chlorine atoms are joined by covalent bonds.
STEP 2 The germanium tetrachloride is distilled off from the mixture.
STEP 3 The germanium tetrachloride is added to an excess of water to produce germanium oxide and hydrochloric acid.
STEPS 1 to 3 are repeated several times.
STEP 4 The pure germanium oxide is reduced by hydrogen to form germanium.
(a) Balance the equation below which represents the reaction in step 1.
GeO2 + ______ HCl → GeCl4 + ______ H2O (1)
(b) Write a word equation for the reaction in step 3.
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Q3. (a) Cola drinks contain phosphoric acid, H3PO4. The two equations show how phosphoric acid can be made from phosphorus.
Balance these two equations.
(i) P4 + ____ O2 → P4O10 (1)
(ii) P4O10 + ________ H2O → 4H3PO4 (1)
Some more practice
4) Mg + O2 → MgO 5) H2 + O2 → H2O 6) Fe + HCl → FeCl2 + H2 7) CuO + HNO3→ Cu(NO3)2 + H2O 8) Ca(OH)2 + HCl → CaCl2 + H2O 9) KHCO3 + H2SO4 → K2SO4 + CO2 + H2O 10) Al + Cl2 → AlCl3
Even more practice - Balancing Equations Game
A-Level question to give a go!
Q11. Copper can be produced from rock that contains CuFeS2
(a) Balance the equations for the two stages in this process.
.....CuFeS2 + .....O2 + .....SiO2 ⟶ .....Cu2S + .....Cu2O + .....SO2 + .....FeSiO3
.....Cu2S + .....Cu2O ⟶ .....Cu + .....SO2
(2)
Formula Literacy
For each of the following compounds;
Identify the number of atoms of each element The formula of the ions it consists of Name it Challenge yourself: calculate its RFM
e.g. the first one is done for you:
1. NaNO3
1 x sodium atom, 1 x nitrogen atom, 3 x oxygen atoms
Na+ and NO3-
Sodium nitrate
Challenge: (1 x 23) + (1 x 14) + (3 x 16) = 85
2. Na2O
3. K3PO4
4. CaBr2
5. Al2O3
6. NH4OH
7. (NH4)2SO4
SI units
To reduce confusion and to help with conversion between different units, there is a standard system of units called the SI units which are used for most scientific purposes. These units have all been defined by experiment so that the size of, say, a metre in the UK is the same as a metre in China. The seven SI base units are:
All other units can be derived from the SI base units. For example, area is measured in square metres (written as m2) and speed is measured in metres per second (written as ms–1). It is not always appropriate to use a full unit. For example, measuring the width of a hair or the distance from Manchester to London in metres would cause the numbers to be difficult to work with. Prefixes are used to multiply each of the units. You will be familiar with centi (meaning 1/100), kilo (1000) and milli (1/1000) from centimetres, kilometres and millimetres.
There is a wide range of prefixes. The majority of quantities in scientific contexts will be quoted using the prefixes that are multiples of 1000. For example, a distance of 33 000 m would be quoted as 33 km.
For the following quantities, which SI unit and most appropriate prefix would you use?
1. The mass of water in a test tube. 2. The time taken for a solution to change colour. 3. The radius of a gold atom. 4. The volume of water in a burette.
5. The amount of substance in a beaker of sugar. 6. The temperature of the blue flame from a Bunsen burner.
Rewrite the following quantities. 7. 0.00122 metres in millimetres 8. 104 micrograms in grams 9. 1.1202 kilometres in metres 10. 70 decilitres in millilitres 11. 70 decilitres in litres 12. 10 cm3 in litres